Question

6.00x10-3 mol of HBr arec

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7 of 14
a Review Constants Periodic Table
Part A
6.00x10-3 mol of HBr are dissolved in water to make 12.0 L of solution. What is the concentration of hydroxide ions,
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Answer 1

The
`[OH^(-)]` is
`2*10^(-11)`

Step-by-step explanation:

Number of moles of HBr=
`6.00* 10^(-3)`

Volume of water = 12.0 L

`[HBr]= (6.00* 10^(-3))/(12)M`

`[H^(+)]= (6.00* 10^(-3))/(12)M`

`[H^(+)][OH^(-)]= 10^(-14)`

`[OH^(-)]= (1.0* 10^(-14))/([(6 *10^(-3))/(12)])= (12 * 10^(-14))/(6 *10^(-3))=2*10^(-11)`

Therefore,
`[OH^(-)]` is
`2*10^(-11)`.